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Total pressure is $2.1 atm$ and equal masses of ${SO}_{2}$ , ${CH}_{4}$ and $O_{2}$ are mixed in an empty container at $298 K$ . Calculate the partial pressure of ${CH}_{4}$ in the mixture. (Assume non reacting mixture)

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Important Questions on States of Matter: Gases and Liquids

MEDIUM

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

A mixture of hydrogen and oxygen contains

40 %

hydrogen by mass when the pressure is

2.2

bar. The partial pressure of hydrogen is bar.

MEDIUM

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

Which one is not correct mathematical equation for Dalton's Law of partial pressure? Here

P =

total pressure of gaseous mixture

HARD

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

The pressure of a moist gas at

27 ° C

4 atm

. The volume of the container is doubled at the same temperature. The new pressure of the moist gas is

\dots \times 10^{- 1}

atm. (Nearest integer)
(Given: The vapour pressure of water at

27 ° C

0.4 atm

)

EASY

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

0.5

moles of gas

A

and

x

moles of gas

B

exert a pressure of

200 P a

in a container of volume

10 m^{3}

1000 K

. Given,

R

is the gas constant in

{JK}^{- 1} {mol}^{- 1}, x

is:

MEDIUM

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

Equal weights of ethane and hydrogen are mixed in an empty container at

25 ° C .

The fraction of total pressure exerted by hydrogen is

MEDIUM

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

The total pressure of a mixture of non-reacting gases

X (0.6 g)

and

Y (0.45 g)

in a vessel is

740 mm

Hg

. The partial pressure of the gas

X

mm

Hg .

(Nearest Integer)
(Given : molar mass

X = 20

and

Y = 45 g {mol}^{- 1}

)

MEDIUM

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

A gaseous mixture of

2

moles of

A

3

moles of

B

5

moles of

C

and

10

moles of

D

is contained in a vessel. Assuming that gases are ideal and the partial pressure of

C

1.5

atm, total pressure is

EASY

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

An ideal gas has pressure

P

, volume

V

and absolute temperature

T

. If

m

is the mass of each molecule and

K

is the Boltzmann constant then density of the gas is

EASY

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

Equal masses of ethane and hydrogen are mixed in an empty container at

298 K

. The fraction of total pressure exerted by hydrogen is

EASY

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

The mole fraction of dioxygen in a Neon-dioxygen mixture is

0.18 .

If the total pressure of the mixture is

25

bar, the partial pressure of neon in the mixture would be

MEDIUM

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

The volume of gas $A$ is twice than that of gas $B$ . The compressibility factor of gas $A$ is thrice than that of gas $B$ at same temperature. What are the pressures of the gases for equal number of moles?

EASY

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

A mixture of

N_{2}

and

Ar

gases in a cylinder contains

7 g

N_{2}

and

8 g

Ar

. If the total pressure of the mixture of the gases in the cylinder is

27

bar, the partial pressure of

N_{2}

is:
[Use atomic masses (in

g {mol}^{- 1}

N = 14, Ar = 40

]

MEDIUM

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

An open vessel at

27^{o} C

is heated until two fifth of the air (assumed as an ideal gas) in it has escaped from the vessel. Assuming that the volume of the vessel remains constant, the temperature to which the vessel has been heated is:

HARD

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

' $x$ ' $g$ of molecular oxygen $(O_{2})$ is mixed with $200 g$ of neon $(Ne)$ . The total pressure of the nonreactive mixture of $O_{2}$ and $Ne$ in the cylinder is $25$ bar. The partial pressure of $Ne$ is $20$ bar at the same temperature and volume. The value of ' $x$ ' is

[Given: Molar mass of $O_{2} = 32 g {mol}^{- 1}$ . Molar mass of $Ne = 20 g {mol}^{- 1}$ ]

MEDIUM

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

Assuming ideal gas behavior, the ratio of density of ammonia to that of hydrogen chloride at same temperature and pressure is: (Atomic weight of Cl is 35.5 u)

EASY

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

300 K

, the density of a certain gaseous molecule at

2

bar is double to that of dinitrogen

(N_{2})

4

bar. The molar mass of the gaseous molecule is

EASY

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

10 moles of a mixture of hydrogen and oxygen gases at a pressure of 1 atm at a constant volume and temperature, react to form 3.6 g of liquid water. The pressure of the resulting mixture will be closest to:

EASY

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

$2 {SO}_{2} (g) + O_{2} (g) \to 2 {SO}_{3} (g)$

The above reaction is carried out in a vessel starting with partial pressure $P_{{SO}_{2}} = 250 m bar$ , $P_{O_{2}} = 750 m bar$ and $P_{{SO}_{3}} = 0 bar$ . When the reaction is complete, the total pressure in the reaction vessel is _____ $m bar$ .

(Round off of the nearest integer).

HARD

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

Liquids

A

and

B

form ideal solution for all compositions of

A

and

B

25^{\circ} C

. Two such solutions with

0.25

and

0.50

mole fractions of

A

have the total vapor pressures of

0.3

and

0.4

bar, respectively. What is the vapor pressure of pure liquid

B

in bar?

EASY

Chemistry>Physical Chemistry>States of Matter: Gases and Liquids>Dalton's Law of Partial Pressure

A mixture of one mole each of

H_{2}

He

and

O_{2}

each are enclosed in a cylinder of volume

V

at temperature T. If the partial pressure of

H_{2}

2 atm,

the total pressure of the gases in the cylinder is:

Total pressure is 2.1 atm and equal masses of SO2, CH4 and O2 are mixed in an empty container at 298 K. Calculate the partial pressure of CH4 in the mixture. (Assume non reacting mixture)

Important Questions on States of Matter: Gases and Liquids

Learn and Prepare for any exam you want !

Total pressure is $2.1 atm$ and equal masses of ${SO}_{2}$ , ${CH}_{4}$ and $O_{2}$ are mixed in an empty container at $298 K$ . Calculate the partial pressure of ${CH}_{4}$ in the mixture. (Assume non reacting mixture)